The Equilibrium Constant

[@alfredlin3637]

This guy is single-handedly keeping my GPA in equilibrium.

[@MegaCadette55]

K

[@LuisMartinez-rg5tr]

+MegaCadette55 HAHA

[@Steelarms]

LOL, dude said "1.0" lmaoo

[@dannyliu257]

Lol I wish I could be as creative as u guys in comments

[@hamdanahmet]

This thread 😆

[@soccerismylife514]

you were there for me when no one else was

[@siobhanquinn4635]

Lol

[@angelado6726]

Omg yes

[@soccerismylife514]

I commented this in undergrad and as a now medical student I can honestly say you are still there for me when no one else is

[@usmanafridix]

Steffy Martinez queen

[@lauramanuel895]

@@soccerismylife514 ohh how cute

[@DannyandPatty]

One thing missing: solid and liquid exceptions.

[@colincaver15]

Was just looking for this to confirm it's real, should be higher in the comments

[@Kim-mu7gw]

solid and liquid should not be included in the equilibrium because only gas has pressure.

[@starf1are505]

Others should know👍

[@laurdesz9050]

@@Kim-mu7gw This is what I was looking for thank you!!!

[@ChuuNebyou]

@@Kim-mu7gw wait what about aq?

[@TheGr1ffinator]

How can he explain things so fast but so well?! Keep up the amazing work Mr Andersen you're the best!

[@nickkraw1]

Thank you Mr. Andersen, your videos are wonderful!

[@thisisnotmyfinalform7856]

Does Kc value tell about the reaction rate???

[@GoodNewsForStrangers]

No it doesn't. Only the concentration of reactants and products. If it's >1 that means there are more products than reactants. We also say that the equilibrium lies on the right. When its

[@shta6400]

@@thisisnotmyfinalform7856 No, it doesn't. It tells us whether we'll have more products or more reactants when we reach equilibrium.

[@shwetakur1]

Thank you soooooo much!!! I love the way you simplify complex concepts and I love the stimulations! I think everyone should watch your videos and benefit from them!!!

[@amrutvani2]

Wow thanx for a beautiful lecture. Never knew the meaning of K value. No chemistry book has shown such simplified meaning.

[@trishalmeida3496]

love this guy's teaching, especially his concise yet detailed explanations. thanks Paul.

[@skiidzman]

I wish he would have covered how to calculate the equilibrium constant...

[@laurdesz9050]

me too man, me too

[@frodobaggins7227]

Products/reactants Equilibrium constant uses molarity so before you set up the equation you need to balance the equation, find the molarity of each product and reactant. Then you set up an equation that multiplies the molarity of all the products with exponents that are the coefficients in the reaction. This has to be over the molarity of the reactants multiplied together with exponents that are the coefficients. Should look like this: (C)^c(D)^d ----------------- (A)^a(B)^b If Keq < 1 it favors reactants in the left direction. If Keq > 1 it favors products in the right direction. By the way solids and liquids are not in the equation.

[@Thekingjuliann]

Bro I a mega test tomorrow and hace to learn this in 4 hours

[@LaLa-he3ln]

@@frodobaggins7227 the molarity, Why multiply without adding up? can you please explain it for me

[@kouchiee]

Equilibrium constant (K) is equal to (C)^c x (D)^d / (A)^a x (B)^b. There is an invisible multiplication sign in the middle, so you have to multiple the molarities/concentrations of the products and divide that over by the molarities/concentrations of the reactants to get K. (And you get molarity by using C = n/V)

[@carolineklevemann2787]

Thank you for helping me through chemistry's difficult concepts. I feel hopeful even when things are hazy in class as I know I can look up the concept on your channel and find clarity! Cheers to you for sharing your knowledge and gift as a teacher!

[@kristianwilliams441]

First your videos helped me with AP biology as a senior in high school. Now they're helping me with chemistry in college. I love these.

[@essammccain9994]

dude i fucking love you

[@istarzgirl]

Thank you! K>1,P>R,arrow points to the right indicating a right shift while K

[@CoDRagna]

hi

[@juliajohnson3494]

Perfect. Just what I needed to share with my students while teaching from home. Thank you for all you do!

[@flakiss997]

I watch your videos all the time, and I would just like to thank you for taking the time to post them. You are an excellent teacher, easy to follow and understand. Once again thank you so much!

[@pboyzzadventures3185]

In equilibrium constant the reaction is reversible hence the double arrows, meaning reactants can be products and products can be reactants. But we try to figure out if we have one more than the other by our constant K. Constant K measures out if we have more reactants or if we have more products at equilibrium. K represents the concentration of our products over our reactants. K>>1 reactant to product, K

[@marklandau365]

i've been watching your videos since my first intro. chem class a 1.5 years ago. i'm in chem 2 now and you are still doing god's work (i'm atheist btw). can't thank you enough for this invaluable resource, sir

[@braedonvangorkom3308]

Thank you sir. Simple, effective, insightful and fun. Just what education should be.

[@srikantadash4603]

Actually I didn't get u yarrr. How can u explain so nicely... Equilibrium constant was a doubt in my mind for 6 years.. U just cleared in a 6 min.... But u r lilbit fast.. I watched at 0.75X .. it was so helpful... Love u bro 😎. From INDIA 🇮🇳

[@Ahnoss]

You're helping me get a degree!

[@dsdsdzxc]

I am poor human being desperate to pass his a level chemistry, but this guy gives me a hope.

[@leann6933]

Mr. Andersen saving my but again. First in high school now in my senior year of college.

[@asifhussain6298]

Daym every problem I have in chem and physics this guy has already done it

[@soap143]

you explain WAYYY better than my chem teacher

[@jeffmartineau8479]

You sir are a gentleman and a scholar

[@teknodisko]

Very helpful! I learned this a week ago and completely forgot the concept. After watching this video however, I was able to jog my memory!

[@Leestella2]

Didn't take chemistry yet, but still understood it. Thanks for the extra knowledge!

[@BrysonRhodesChannel]

you are super helpful man bless you and all the generations that come behind you!

[@rmulenga]

At 3 min, the expression should be aA + bB cC + dD (missing PLUS sign on RHS)

[@bongplayda8178]

Thank you Mr. ANderson...I have watched your videos lately and I really learned a lot

[@anas8296]

this guy proceeds to explain in 6 minutes what my professor failed to explain in 4 hours

[@dooham1383]

Thank you for the videos! Really clarified important concepts!

[@royc7421]

Wish they had KZbin videos when I was in college taking chemistry.

[@codezmister]

The song in the beginning of the video is so cool!

[@theFLacker123]

The illustrations are very helpful for me. It would be helpful if they just called it the equilibrium ratio constant.

[@alphanguyen2901]

u r the goat & teach sm better than my teacher thank u sir

[@chitranjansingh2196]

You teach very well. I like your teaching

[@KC-ke1vp]

oh my! thank you sm! hoping it will help me in my prelim exam in cellular and molecular biology!! taking the test in a few! ❤️‍🔥

[@sukitvirathana7151]

you just practically save my life

[@xisaabtv8082]

Thank you very much. You say if Kc is greater than 1, it moves from reactants to the products side. And if the Kc is less than 1, it moves products to reactants. My question is when can we have the equilibrium mixture for an appreciable concentration of both reactants and products ?

[@micahbendicion8444]

4:03 You said "standard temperature and pressure", but then the box said 25 degrees Celsius, which is room temperature. Which did you intend?

[@yahiazaatit7679]

overall the chemical reaction's entourage

[@mattpresti9456]

Always enjoy these videos. I am still confused on one thing. At nine minutes during an ICE table the change in H2O is shown as .038 mols. The initial value is zero and the equilibrium value is .138. So why is the change not .138?

[@harryli7557]

and here I am a college junior coming back to this yet again

[@TheLivirus]

Thanks! You make the whole thing very understandable.

[@sheikhs.mahmud4020]

Of course that was helpful...thanks! You are the best, Andersen..

[@nasgrp2437]

mr anderson can you do more practiced questions and examples please???

[@twokidsmovies]

So is the K value the same as Log K? Like when modeling in the GWB, each reaction has Log K values at different temperatures

[@abdulrehmankhan3428]

Thanks Mr.Andersen this is really helpful

[@pofficial-qi6es]

Very very helpful thanks... And very easy language....

[@tyson6695]

I already knew how to solve it,but the question that was annoying me was that what is k constant and what does its value represent,thanks very much sir,definitely subscribing👍👍👍👍

[@samuelhodgesv9532]

Your videos are so helpful! Thanks so much! Keep up the good work.

[@Creacion83]

CO2 (g) + H2O (l) H2CO3 (aq) Calculate the equilibrium constant using the following concentrations [H2CO3] = 7.75 x 10-4 M and [CO2] = 5.65 x 10-1 M

[@anthonyokpara2117]

am finally getting smething BOZEMAN yuh the best...thkz alot

[@nasgrp2437]

+Anthony okpara or that your just dumb and took this guy for u to actually get something and get you to use one of your brain cell on

[@krystelshaynelantano6348]

how did you get the numerical value of the constant?

[@streamleazefishhouse]

+Krystel Shayne Lantano I would like that as well :) Did you find the answer?

[@OOOOOO-dx7zu]

+Krystel Shayne Lantano you use the concentrations, or you can get it experimentally, i think

[@CoDRagna]

uh didnt you watch the video? concentrations in products / concentration in reactants but make sure you multiply them and properly exponentiate them to their coefficient. those values will be given in a problem or determined experimentally. you asked this 2 years ago so i doubt you give a rats ass about the answer now

[@chrisfrost7945]

@@CoDRagna I care

[@CoDRagna]

@@chrisfrost7945 great point!

[@anthonyrichard1365]

Great video! I wonder why the temperature has an impact on what will be produced more, the reactant or the product, and therefore, what the K value is. What role does temperature play in the way that at one moment the product can be produced more than the reactant (thus, favoring the forward reaction)? Conversely, how does a lower temperature of the same reaction make it favor the reverse reaction?

[@eleanormystim1641]

Thanks so much, got Chem sac tomorrow and I finally understand the concept :)

[@queenzht]

Time to review ... Thank you for your video.

[@Christaxio]

Fantastically explained!

[@Niki-cf3tr]

Thank you so much I really needed this 🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻

[@farouqalsalih619]

If a reaction has a very low K value, would that mean that the reaction at that temperature is non spontaneous as there are very few products. Also, if the k value is very large, would that mean that the reaction is spontaneous as there are many products?

[@marvinabuli4487]

can you do a video on how to find the equilibrium constant in electrolysis

[@madisonpage5661]

4:26 Why does the increase in temperature decrease the K value?

[@judeabughalia9225]

depends on the forward reaction, if its exothermic (which is the case for most reactions) then clearly if u increase the temperature the equilibrium will favor the endothermic reaction (which is the backward reaction) which increases the reactants, making the K value lower. i hope that was helpful!!

[@janahany1481]

THANK YOU SOO MUCH I LOVE YOUR VIDEOS THEY ARE SUPER HELPFUL

[@rede_neural]

I don't know why use concentrations for this, I think molar fractions would be better. If there is an equal amount of products and reactants, but there molar masses aren't equal, then k won't be equal to one, but it should.

[@100percentjoy]

Thank you Mr. Anderson

[@ahuman9113]

Still got a 62 on my test👍

[@Spiceodog]

Somehow my chemistry teacher was able to teach me this is 27 minutes, and I only understood about 20% of what he said

[@gingerlove9085]

is it the same if it ask you to writ an equation for equilibrium constant for forward reaction

[@samsunnahar9175]

Thanks a lot for your clear explanation!

[@crazyotaku5754]

excellent.... splendid explanation

[@normalperson5317]

It was really helpful. keep going!

[@Scan420]

God damn. How did he explain like that in 6 minutes

[@brettstefanishin574]

Wow thanks! That was so helpful!

[@annnee6409]

You went through very well the meaning of k, but you didn't go through how you got to value eg what did you calculate eg what were the concentrations?

[@clairenime]

Thank you sooooo much, great videos

[@matildemateus3977]

Hi, I just have one doubt: why do we multiply ( the products by the products and the reactants by the reactants) instead of adding, when calculating the equilibrium constant?

[@ajsim]

Very helpful. Great job, and thank you!

[@ASteel-yo8em]

Thank you very much for this helpful video!

[@aneeshvaidya7838]

Thank you soooooooooo much. U r an amazing teacher.

[@Creacion83]

Calculate the equilibrium constant using the following concentrations [H2CO3] = 7.75 x 10-4 M and [CO2] = 5.65 x 10-1 M.

[@satinderjit4]

Would need a balanced equation since the coefficients can change the equilibrium constant. For example, the equilibrium constant would be different if one of the balanced equation coefficients was 1/2 compared to a 2.

[@schnarfel]

thank you! it feels like you did it all on one breath though!

[@mybirjitthangjam7388]

Tkkk.....very must sir. Love from Manipur

[@msabbasi01]

How can we solve units of concentration for the followinv reaction? I have tried so hard on it but couldn't understand that how do we get moldm‐³ as its answer. When nitrogen reacts with hydrogen to form ammonia, the equilibrium mixture contains 0.31 mol dm‐³ and 0.50 mol dm‐³ of nitrogen and hydrogen respectively. If the Kc is 0.50 mol‐²dm⁶, what is the equilibrium concentration of NH3?

[@huzaimkhan9347]

When Kc isn't equally to 1,then it means the system isn't in equil.state then why the constant is called EQUILIBRIUM constant.

[@michaelmcfarlane3067]

thank you so much!!! you are a great teacher!!!!

[@TheBabyLioness]

man this was soooo helpful! thanks!!

[@princessmary103]

Love this. Thank you

[@mosessaleh6406]

Very helpful, thank you

[@dakhemyst]

Excellent. Thank you

[@T12J7]

Nice video, but it did not answer the fundamental questions regarding equilibrium constant: 1. why is it calculates the way it is and 2. for what does the value stand for? 1. So equilibrium constant is calculated with the formula K = ([C]^c * [D]^d) : ([A]^a * [B]^b) Why is it calculated like this? Why is it not calculated like this: K = (c*[C] * d*[D]) : (a*[A] * b*[B]) or like this K = (c*[C] + d*[D]) : (a*[A] + b*[B]) or like this K = ([C]^c + [D]^d) : ([A]^a + [B]^b) or just like this K = ([C] + [D]) : ([A] + [B]) ? Why does it have to be like it is, and why would these other calculations not good enough when determinating the ratio between the starting compounds of the reaction and the product compounds of the reaction? 2. The value of K is not the concentration ratio between the starting compounds of the reaction and the product compounds of the reaction, because that would be calculated just with a simple formula: K = ([C] + [D]) : ([A] + [B]) So, why is K calculated like it is, and what does it's number really stand for?

[@Nowogo]

this guy is awesome

[@QUITEthegamer]

this was just beautiful!!!

[@Mochibitz]

So, we can't calculate for K? It would always be given to us?

[@sehmio]

This was so helpful!! Thank you so much :)

[@judeabughalia9225]

i legit asked my teacher what K actually is, like what does it mean and why we use it. her reply, "we already covered it in class. i suggest you go over the chapter again!!!!" I wanted to throw something at her istg

[@Anni6758]

Can anyone help me understand why "there are 2 moles of water" in the equation which says 2H2O - I thought this meant there were 2 molecules of water (and moles is like 6 x 10^23)

[@johndereksanglay4232]

I have an upcoming report for this topic and thnks god that you creaed this video. 😇

[@bhartihooda963]

Thanx it helps in my AIIMS questions

[@BigChungusthe3rd]

How does temperature affect the equilibrium constant?

[@alandawat6476]

thank you so much but i have a question! we dont write the liquids and solids in the equation becuz it doesnt affect the concentration but what about aqueous substances? do we include them in the equation? does it affect the concentration